Objectives Explain why atoms form bonds Define chemical

Objectives Explain why atoms form bonds Define chemical bond & name three types of chemical bonds Bonding Atoms Why do atoms bond? - each atom wants a full outermost energy level

- gain, lose, and share valence electrons to achieve the duet or octet rule aka: being happy - ex. Group 18: He, Ne, Ar Chemical Bonds Chemical Bonds - attractive force that holds atoms or ions

together - 3 types - determines the structure of compound - structure affects properties - Chemical Structure/Models Chemical Structure/Molecular Models

- arrangement of bonded atoms or ions : the average distance between the nuclei of two bonded atoms : the angle formed by two bonds to the same atom Molecular Models of Compounds - atoms are represented by balls

- bonds are represented by sticks * good for seeing angles - chemical symbols represents atoms - lines are used to represent bonds * good for seeing angles H H

O Molecular Models Cont. Space filling - colored circles represent atoms, and the space they take up - no bonds, no bond angles Electron Dot/Lewis Structure - chemical symbol represent atom

- dots represent valence electrons - 2 center dots represent a bond - no bond angles, no bond length Objectives Describe how an ionic, covalent and metallic bonds forms Relate the properties of ionic compounds to the structure of crystal lattices

Compare polar and non polar bonds, and demonstrate how polar bonds affect polarity of a molecule Describe the structure and strength of bonds in metals & relate their properties to their structure Ionic Bonds / Ionic Compounds Definition - bond formed by the attraction between oppositely

charged ions cation: anion: - oppositely charged ions attract each other and form an ionic bond ex. Na+ + Cl- = NaCl - electrons are transferred from one atom to another - negative ions attract more positive ions, and soon a network is formed

Networks / Crystal Lattices Networks ex. NaCl - every Na ion is next to 6 Cl ions - strong attraction between ions creates a rigid framework, or lattice structure: aka: crystals ex, cubes, hexagons, tetragons

Properties of Ionic Compounds Structure affects properties - strong attractions between ions: strong bonds - high melting/boiling pt - shatter when struck (think of it as one unit) - conductivity : ions are so close together, fixed positions, (cant move)

NO conductivity : ions are freely moving due to a broken lattice structure Good conductivity Covalent Bonds Definition - can be a single, double, or triple bond single, 2e-s (-); double, 4e-s (=); triple, 6e-s( )

- always formed between nonmetals - mostly low melting/boiling points 2 types of bonds - polar - non polar Covalent Bond Cont. - bonded atoms that share e-s equally - same atoms bonded

ex. Cl Cl: Cl2 - bonded atoms that do not share e-s equally - different atoms bonded H ex. H N H: NH3 Metallic Bonds Definition -

Properties - Conductivity: Good: electrons can move freely - Malleable: lattice structure is flexible Predicting Bond Type

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